EBK EXPLORING CHEMICAL ANALYSIS
EBK EXPLORING CHEMICAL ANALYSIS
5th Edition
ISBN: 8220101443908
Author: Harris
Publisher: MAC HIGHER
Question
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Chapter 17, Problem 17.13P

(a)

Interpretation Introduction

Interpretation:

Moles of H2 produced has to be calculated.

Concept Introduction:

Moles of ideal gas present in a gas container are calculated by the following equation as follows:

    n=PVRT

Here,

n is mole of ideal gas.

P is pressure.

V is volume.

T is temperature in Kelvin scale.

R is the universal gas constant.

(a)

Expert Solution
Check Mark

Answer to Problem 17.13P

1.9473×103mol hydrogen gas is produced.

Explanation of Solution

Formula to calculate moles is as follows:

  n=PVRT        (1)

Substitute 303K for T, 0.996bar for P, 0.082Latmmol-1K-1 for R , and 49.22mL for V in equation (1).

  MolesofH2gas=(0.996bar)(49.22mL)(0.082Latmmol-1K-1)(303K)=(0.996bar)(1atm1.01325bar)(49.22mL)(1L1000mL)(0.082Latmmol-1K-1)(303K)=1.9473×103mol

Hence, number of moles is 1.9473×103mol.

(b)

Interpretation Introduction

Interpretation:

Concentration of EDTA in molarity has to be determined.

Concept Introduction:

In analytical chemistry, coulometric titration is a method in titrating agent is produced in solution by electrolysis. Amount of that substance is determined by measuring the quantity of electricity used to electrolyze that substance. For coulometric titration, no standard solution is needed.

Moles of electron flow in a coulometric titration is calculated by the equation as follows:

    Molesofelectronflow=(Electriccurrent)(time)Faradayconstant

(b)

Expert Solution
Check Mark

Answer to Problem 17.13P

Concentration of EDTA solution is 0.04112M.

Explanation of Solution

Reduction reaction of water molecule to form hydrogen gas is written as follows:

    2H2O+2e2OH+H2

Here total number of electrons flow has taken place is calculated as follows:

    Molesofelectronflow=(2)(Moleofhydrogengasproduced)=(2)(1.9473×103mol)=3.8946mol

As EDTA is a two-electron donor, so concentration of EDTA solution can be calculated as follows:

    ConcentrationofEDTAsolution=(3.8946×103mol2)(47.36mL)(1L1000mL)=0.04112M

Hence, concentration of EDTA solution is 0.04112M.

(c)

Interpretation Introduction

Interpretation:

Time required for electrolysis has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Expert Solution
Check Mark

Answer to Problem 17.13P

Time taken for electrolysis is 4.75hr.

Explanation of Solution

Formula to calculate time is as follows:

  timeinsecond=(Molesofelectronflow)(Faradayconstant)(Electriccurrentinamperes)        (2)

Substitute 3.8946×103mol for moles of electron flow, 96485Cmol1 for faraday constant and 0.02196A for electric current in equation (2).

    timeinsecond=(3.8946×103mol)(96485Cmol1)(0.02196A)=17111.59s=4.75 hour

Hence, time taken for electrolysis is 4.75 hour.

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